1 / 4

25.0 g

25.0 g of copper (II) oxide, Cu 2 O, reacts with hydrogen to produce copper metal and water. How many grams of copper are produced. CuO + H 2 → Cu + H 2 O. 1. 1. ?g. = 20.0 g Cu. 25.0 g. Cu = 64 O = 16 80g/mole.  80g/mole. x 64 g/mole.

ismet
Download Presentation

25.0 g

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. 25.0 g of copper (II) oxide,Cu2O, reacts with hydrogen to produce copper metal and water. How many grams of copper are produced.CuO + H2→ Cu + H2O 1 1 ?g = 20.0 g Cu 25.0 g Cu = 64 O = 16 80g/mole  80g/mole x 64 g/mole Quiz instructions: Underline the important facts and set up the problem. Honor’s students solve the problem. Lab 30 will not be accepted after today. We will do Lab 25 Wed, and Friday; Notebook due again Wed. 0.313 mole 0.313 mole

  2. Ammonia is synthesized from hydrogen and nitrogen according to the following equation: N2 + 3 H2→ 2NH3 If an excess of nitrogen is reacted with 6.82 g of nitrogen, how many grams of ammonia can be produced. N2 + 3 H2→ 2 NH3 2 1 N = 14.0 3H = 3.0 17.0 g/mole ?g = 8.28 g NH3 6.82 g 28.0 g/mole N2 x 17.0g/mole 0.244 mole 0.487 mole

  3. Assume that in the decomposition of potassium chlorate, KClO3, 85 g of O2 form. How many grams of potassium chlorate were used? 2 2 K+Cl- + O2 2 KClO3 3 3 85 g ?g = 520 g KClO3 K =39 Cl = 35 O = 3x16.0 = 48 122g/mole 32 g/mole x 122 g/mole 2.5 mole 4.2 mole

  4. Stoichiometry: Vocabulary positive charges equal negative charges • Balanced Chemical Formula • Balanced Chemical Equation • grams • moles • “known” • “unknown” • gram formula weight (gfw) or gfm • mole ratio All atoms in reactants are present in the same quantity in the products measurement of mass quantity of particles of a substance The “given quantity” The “quantity” you are being asked to find The mass found in one mole of a substance A comparison between the coefficients of the “known” and the “unknown” expressed as a fraction.

More Related